Answer:
0.315 atm
Explanation:
PV = nRT
P(96.2) = (1.24)(0.08206)(25 + 273)
P = 0.315 atm
Nitrogen combine with hydrogen to produce ammonia
at a
ratio:

Assuming that the reaction has indeed proceeded to completion- with all nitrogen used up as the question has indicated.
of hydrogen gas would have been consumed while
of ammonia would have been produced. The final mixture would therefore contain
Apply the ideal gas law to find the total pressure inside the container and the respective partial pressure of hydrogen and ammonia:
Answer:
See explaination
Explanation:
Please kindly check out the attached files for the curved-arrow mechanism for the Claisen condensation of ethyl ethanoate treated with ethoxide ion.
<h2>YOUR ANSWER Is number of istopes</h2>
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Answer:
- Partial pressure He = 276 torr
- Partial pressure Ar = 457 torr
- Total pressure = 733 torr
Explanation:
Assuming temperature remains constant, we can use Boyle's law to solve this problem: P₁V₁=P₂V₂.
Once the two flasks are connected and the stopock opened, the total volume is:
Now we use Boyle's law <em>twice</em>, to <u>calculate the new pressure of </u><em><u>each</u></em><u> gas</u>:
- He ⇒ 752 torr * 275 mL = P₂He * 750 mL
P₂He = 276 torr
- Ar ⇒ 722 torr * 475 mL = P₂Ar * 750 mL
P₂Ar = 457 torr
Finally we <u>calculate the total pressure</u>, adding the partial pressures:
- Total pressure = P₂He + P₂Ar = 733 torr